ARTICLE pubs.acs.org/IC
Lanthanoid-Containing Open WellsDawson Silicotungstates: Synthesis, Crystal Structures, and Properties Lubin Ni,† Firasat Hussain,†,‡ Bernhard Spingler,† Stephen Weyeneth,§ and Greta R. Patzke*,† †
Institute of Inorganic Chemistry, University of Zurich, Winterthurerstrasse 190, CH-8057 Zurich, Switzerland Department of Chemistry, University of Delhi, 110 007 Delhi, India § Physik-Institut der Universit€at Z€urich, Winterthurerstrasse 190, CH-8057 Z€urich, Switzerland ‡
bS Supporting Information ABSTRACT: Five novel lanthanoid-containing silicotungstates with polymeric crystal structures [Ln2(H2O)7Si2W18O66]n10n [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5 (C2H4O2)0.5Si2W18O66]n10n were obtained from the one-step reaction of Na10[SiW9O34] 3 nH2O with Ln(NO3)3 3 nH2O in a sodium acetate buffer. The compounds were characterized by single-crystal X-ray diffraction and a wide range of analytical methods, including FT-IR, UV/vis, and photoluminescence spectroscopy as well as electrochemistry and thermogravimetric analysis. This new polyoxotungstate series is the first example of lanthanoids embedded in the open WellsDawson silicotungstate anion [R-Si2W18O66]16. The lanthanoid-containing Wells Dawson-type polyoxoanions [Ln2(H2O)7Si2W18O66]10 [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5 (C2H4O2)0.5Si2W18O66]10 are linked by Ln3þ cations to form 3D architectures for Gd-1 or 2D frameworks for the isostructural compounds Tb-2, Dy-2, Ho-2, and Gd-2. The structure-directing influence of the lanthanoid cation on the local structure of the dimeric building blocks and on the crystal packing motifs is investigated in detail. The photoluminescence properties of Tb-2 and Dy2 were investigated at room temperature, and Ho-2 exhibits an interesting photochromic behavior. The magnetic susceptibility of Gd1 and Gd-2 was studied in the temperature range between 2 and 300 K for its effective magnetic moment.
’ INTRODUCTION Polyoxometalates (POMs) are transition-metal oxide nanoclusters (usually of V, W, and Mo in their high oxidation states) that provide an exceptional variety of structural motifs from solution-based approaches in aqueous media. The manifold potential POM applications arising from their infinite number of molecular architectures are now widely investigated, e.g., in the fields of medicine, catalysis, water splitting, imaging techniques, multifunctional materials, or bio- and nanotechnology.113 Lanthanoid-containing POMs are of special interest with respect to key magnetic properties, luminescence, and Lewis acid catalysis, and Gd POMs, in particular, are used for the development of magnetic resonance imaging agents.14 We have thus explored the reactivity of lanthanoid cations with different types of lacunary POMs,15 and this synthetic strategy has proven rather fruitful: First, lacunary POMs and large oxophilic lanthanoid cations can be readily combined into high nuclear polyoxoanion complexes with unprecedented structures, sizes, and new properties. Second, lanthanoid cations are particularly efficient linkers because of their high coordination numbers and flexible coordination geometries. Therefore, this method is generally favorable for constructing polymeric or unusually large POM assemblies. This is illustrated by Pope et al.’s high-nuclear cerium-containing polyoxotungstoarsenate(III) [Ce16As12(H2O)36W148O524]76, which has long been the largest polyoxotungstate ever observed,16 r 2011 American Chemical Society
followed by Kortz et al.’s synthesis of [Ce20Ge10W100O376 (OH)4(H2O)30]56.17 Recently, our group has amplified the spectrum of lanthanoid linkers to middle and late members of the series,18 as represented by the [Cs⊂Ln6As6W63O218(H2O)14 (OH)4]25 type (Ln = Eu, Gd, Tb, Dy, Ho, Er) and the [Gd8As12W124O432(H2O)22]60 polyanion.15a,b Our efforts finally resulted in the [Ln16As16W164O576(OH)8(H2O)42]80 (Ln = Eu, Gd, Tb, Dy, Ho) family with the largest number of tungsten centers to date.15c Related studies are performed by the groups of M€uller, Francesconi, Yamase, Krebs, Kortz, Gouzerh, Secheresse, Hill, and others.19 As shown in our present work, however, the inexhaustible structural variety of lanthanoid-containing POM structures, ranging from discrete building blocks to polymeric arrangements, can only be tapped by a comparable flexibility of synthetic approaches. Although the reactivity of the monovacant silicotungstate [SiW11O39]8 with trivalent lanthanoids leading to the formation of 1D inorganic chains or 2D layers has been well investigated by Peacock,20 Pope,21 Mialane,22 Kortz,23 and Niu24 and their respective co-workers, no studies on the conversion of the trilacunary Keggin polyoxoanion [SiW9O34]10 into WellsDawson [Si2W18O66]16 ions in the presence of lanthanoid cations have been reported. Furthermore, only a few 3D inorganic Received: January 27, 2011 Published: May 10, 2011 4944
dx.doi.org/10.1021/ic2001943 | Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry architectures of lanthanoid-containing POMs are known up to now. Two Keggin-type monolacunary polyoxotungstoborates [Ln(H2O)(BW11O39H)]10 (Ln = Ce, Nd) have been recently discovered by An and co-workers.25 In the following, we report on the reactivity of the [A-R-SiW9O34]10 precursor in the presence of different lanthanoid cations. We successfully obtained five polymeric Ln-based POMs (Ln = Gd, Tb, Dy, Ho) from the incorporation of lanthanoid cations into the open WellsDawson anion [R-Si2W18O66]16, which was first characterized by Herve et al.26,27 The potassium salt of [Si2W18O66]16, furthermore, serves as a precursor for the formation of the silicotungstate polyanions R-[{[K(H2O)2(μ-H2O)-[Li(H2O)2]}2Si4W36O126(H2O)2]16 and R-[{[K(H2O)][K(H2O)4]}2Si8W36O136]22 through a stepwise self-assembly process.28 The open Wells Dawson anion can intercalate two transition-metal cations (Mn, Co, Ni, Cu) in addition to the Kþ ion present in the pocket, resulting in different coordination modes28 (cf. Table S1 in the Supporting Information for a survey of related compounds). Later, Herve and co-workers accessed polyanions with dinuclear {KV2O(H2O)2}5þ and tetranuclear {Fe4(OH)6}6þ moieties included in the pocket between the two [R-Si2W18O66]16 subunits through reaction of the open WellsDawson anion with VV and FeIII cations.29 In 2004, Kortz et al. synthesized a pentacoppersubstituted polyanion, with the copper oxo cluster {Cu5(OH)4 (H2O)}6þ perfectly fitting into the cavity of the open Wells Dawson anion.30 The same group also discovered monosubstituted transition-metal derivatives of γ-[Si2W20O70]12.31 The title compounds are all constituted of the novel dimeric polyoxoanion [Ln2(H2O)7Si2W18O66]10 [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5(C2H4O2)0.5Si2W18 O66]10, respectively, which consist of two lanthanoid cations within the open WellsDawson units. These polyoxoanion moieties are further linked by Ln3þ cations into 3D or 2D architectures. The influence of the cationic radii on the local structure of the POM as well as on the 3D packing motifs of the compounds is discussed. The photoluminescent properties of the terbium- and dysprosium-containing polyanions were investigated at room temperature. All compounds were electrochemically characterized in a sodium acetate buffer (pH 4.4) solution as the supporting electrolyte.
’ EXPERIMENTAL SECTION Materials and Analytical Methods. The Na10[A-R-SiW9O34] 3 23H2O precursor was prepared according to literature protocols32 and characterized with IR spectroscopy. All other chemicals were commercially purchased and used without further purification. Elemental analyses of all polyanions were performed by Mikroanalytisches Labor Pascher, Remagen, Germany. Fourier transform infrared (FT-IR) spectra were recorded on a Perkin-Elmer BXII spectrometer with KBr pellets. Thermogravimetric analysis (TGA) measurements were performed on a Netzsch STA 449 C between 30 and 800 °C with a heating rate of 5 K min1 in a nitrogen atmosphere. UV/vis spectra were recorded on a Perkin-Elmer Lambda 650S spectrometer. Powder X-ray diffraction (PXRD) data were recorded on a Philips X0 Pert PRO diffractometer, operated at 40 kV and 30 mA (Cu KR1 radiation). Photoluminescence measurements were performed on a Perkin-Elmer LS 50B spectrometer. Magnetic measurements were performed with a SQUID magnetometer (Quantum Design, MPMS-7) in the temperature range 2300 K with an applied magnetic field of 2 kOe. Here a small temperature-independent contribution to the paramagnetic susceptibility, stemming from the electronic susceptibility of the sample and from the sample holder
ARTICLE
configuration, was subtracted from the data prior to further analysis (1.54 103 emu Oe1 mol1 for Gd-1 and 5.38 104 emu Oe1 mol1 for Gd-2). Cyclic voltammetry (CV) measurements were performed using a Metrohm Computrace model 757 VA voltammetric analyzer. The system was operated using 757 VA Computrace software (Metrohm). The three-electrode cell system consisted of a 2 mm glassy carbon working electrode (modified or unmodified), a saturated Ag/AgCl reference electrode, and a platinum wire counter electrode.
Synthesis of Na2CsCaGd2[Gd2(H2O)7Si2W18O66]Cl 3 27H2O (Gd-1). A total of 0.369 g (0.150 mmol) of Na10[SiW9O34] 3 23H2O
was dissolved in 25 mL of a sodium acetate buffer (pH 4.4) with stirring. A total of 0.203 g (0.450 mmol) of Gd(NO3) 3 6H2O was slowly added to the reaction mixture. The solution was stirred continuously at 80 °C for 90 min, followed by cooling to room temperature and filtering. The addition of a 1.0 M CsCl solution (0.5 mL) to the colorless filtrate and slow evaporation at room temperature led to the formation of colorless needlelike crystals after about 1 week. Yield: 21.0% (based on Na10[A-RSiW9O34] 3 23H2O). FT-IR (cm1): 1001 (s), 938 (s), 871 (vs), 833 (s), 808 (s), 723 (s), 555 (w), 529 (w). Elem anal. Calcd (found): W, 55.92 (55.20); Gd, 10.63 (11.00); Cs, 2.25 (3.10); Na, 0.78 (0.63); H, 1.16 (1.13). The number of water molecules has been confirmed by TGA (cf. Figure S5 in the Supporting Information).
Synthesis of Na2Cs3H2Tb[Tb2(H2O)7Si2W18O66] 3 17H2O (Tb-2). The above synthetic procedure was modified by using 0.196 g (0.450 mmol) of Tb(NO3)3 3 5H2O instead of Gd(NO3)3 3 6H2O. Colorless block-shaped crystals were obtained after about 1 week. Yield: 13.8% (based on Na10[A-R-SiW9O34] 3 23H2O). FT-IR (cm1): 1002 (s), 937 (s), 876 (vs), 818 (s), 718 (s), 547 (w), 524 (w). Elem anal. Calcd (found): W, 57.28 (54.20); Tb, 8.25 (8.77); Cs, 6.90 (6.74); Na, 0.80 (1.00); H, 0.87 (0.99). The number of water molecules has been confirmed by TGA (cf. Figure S5 in the Supporting Information).
Synthesis of Na4Cs3DyH[Dy2(H2O)6.5(C2H4O2)0.5Si2W18O66] Cl 3 17H2O (Dy-2). The above synthetic procedure was applied using
0.197 g (0.450 mmol) of Dy(NO3)3 3 5H2O instead of Gd(NO3)3 3 6H2O. Colorless blocklike crystals were obtained after about 1 week. Yield: 15.2% (based on Na10[A-R-SiW9O34] 3 23H2O). FT-IR (cm1): 1002 (s), 940 (s), 882 (vs), 817 (s), 716 (s), 551 (w), 528 (w). Elem anal. Calcd (found): W, 56.19 (53.30); Dy, 8.27 (8.11); Cs, 6.77 (7.05); Na, 1.56 (1.61); H, 0.85 (0.99); C, 0.20 (0.16). The number of water molecules has been confirmed by TGA (cf. Figure S5 in the Supporting Information).
Synthesis of Na4Cs3Ho[Ho2(H2O)7Si2W18O66] 3 18H2O (Ho-2).
The above synthetic procedure was performed with 0.200 g (0.450 mmol) of Ho(NO3)3 3 5H2O instead of Gd(NO3)3 3 6H2O. Light-pink block-shaped crystals were obtained after about 1 week. Yield: 12.4% (based on Na10[A-R-SiW9O34] 3 23H2O). FT-IR (cm1): 1003 (s), 939 (s), 868 (vs), 833 (s), 809 (s), 714 (s), 555 (w), 529 (w). Elem. anal. Calcd (found): W, 56.50 (54.00); Ho, 8.44 (8.68); Cs, 6.81 (6.68); Na, 1.57 (1.58); H, 0.86 (0.98). The number of water molecules has been confirmed by TGA (cf. Figure S5 in the Supporting Information).
Synthesis of Na2.5Cs3.5GdH2[Gd2(H2O)7Si2W18O66](C2H3O2) 3 16H2O (Gd-2). The synthetic procedure was conducted as described
above for Gd-1 with one alteration: instead of 0.5 mL of a 1.0 M CsCl solution, 1.2 mL was added to the colorless filtrate dropwise. Colorless blocklike crystals were obtained after about 1 week. Yield: 15.6% (based on Na10[A-R-SiW9O34] 3 23H2O). FT-IR (cm1): 1002 (s), 934 (s), 886 (vs), 814 (s), 720 (s), 551(w), 529(w). Elem anal. Calcd (found): W, 56.17 (54.50); Gd, 8.00 (7.68); Cs, 7.30 (7.41); Na, 0.97 (1.09); C, 0.41 (0.40); H, 0.86 (0.70). The number of water molecules has been confirmed by TGA (cf. Figure S5 in the Supporting Information). X-ray Crystallography. Data collection of compounds Gd-1, Gd2, Tb-2, Dy-2, and Ho-2 was performed on an Oxford Xcalibur Ruby CCD single-crystal diffractometer (Mo KR radiation, λ = 0.710 73 Å) at 183(2) K. Lorentz and polarization corrections were applied, and an 4945
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Table 1. Crystallographic Data for Compounds Gd-1, Gd-2, Tb-2, Dy-2, and Ho-2 Gd-1 empirical formula
CsCaH68Na2Gd4
Gd-2 C2Cs3.5H51Gd3Na2.5
O100Si2W18Cl
a
Tb-2 Cs3H50Na2Tb3
O91Si2W18
Dy-2 CCs3H50Dy3Na4
O90Si2W18
Ho-2 Cs3H50Ho3Na4
O90.5Si2W18C1
O91Si2W18
fw (g mol1)
5917.18
T (K)
183(2)
183(2)
183(2)
183(2)
183(2)
λ (Å)
0.710 73
0.710 73
0.710 73
0.710 73
0.710 73
5890.84
5777.10
5888.93
5857.12
cryst syst, space group
monoclinic, C2/c
triclinic, P1
triclinic, P1
triclinic, P1
triclinic, P1
a (Å)
26.1719(4)
12.8242(1)
12.9462(2)
12.8335(3)
12.9422(12)
b (Å) c (Å)
20.7408(4) 39.3620(8)
15.7895(2) 23.2486(3)
15.7702(2) 23.1831(3)
15.7343(3) 23.1443(4)
15.6464(8) 23.0735(12)
R (deg)
90.00
99.591(1)
99.135(1)
99.304(2)
99.062(4)
β (deg)
94.021(2)
97.904(1)
98.002(2)
98.206(2)
98.117(6)
γ (deg)
90.00
91.547(1)
93.398(1)
92.871(2)
93.777(6)
V (Å3)
21314.1(7)
4591.65(9)
4611.6(1)
4551.9(1)
4549.2(5)
Z
8
2
2
2
2
abs coeff (mm1)
22.476
26.064
25.939
26.248
26.318
dcalcd (Mg m3) F(000)
3.719 20756
4.307 5141
4.263 5116
4.293 5085
4.226 4992
cryst size (mm)
0.38 0.06 0.04
0.15 0.08 0.05
0.23 0.22 0.13
0.23 0.18 0.06
0.11 0.09 0.08
GOF on F2
0.885
0.996
1.065
0.921
0.916
R1 [I > 2σ(I)]a
0.0490
0.0384
0.0414
0.0401
0.0515
wR2 [I > 2σ(I)]a
0.0914
0.0906
0.0986
0.0837
0.1075
R1 = ∑(Fo Fc)/∑Fo and wR2 = {∑w(Fo2 Fc2)2/∑w(Fo2)2}1/2.
absorption correction was performed using the program CrysAlis.33 Direct methods were used to locate the heavy-metal atoms (SHELXS97). The remaining atoms were located from successive Fourier maps (SHELXL-97).34 Further details on the crystal structure data can be obtained from ICSD/FIZ Karlsruhe via www.fiz-karlsruhe.de/icsd.html [fax (þ49) 7247-808-666; e-mail
[email protected]], on quoting the depository numbers CSD 422265422268 for Gd-1, Tb-2, Dy-2, and Ho-2, respectively, and 422404 for Gd-2. All heavy atoms were refined anisotropically except for some disordered alkali-metal counterions and free water molecules. The incorporation of one calcium cation into Gd-1 was deduced from the crystallographic environment of this specific position. Because the calcium content determined from experimental analyses is considerably lower, the selected single crystal probably deviates in this minor detail from the bulk material that is otherwise in good agreement with elemental analysis results for the main constituting elements. As a consequence, the experimental PXRD of Gd-1 (Figure S10 in the Supporting Information) does not display a very convincing match with the theoretical pattern calculated from the X-ray crystallographic data. It is also noteworthy that the PXRD of Gd-1 displays the lowest crystallinity among the series (cf. Figures S10S14 in the Supporting Information), which is in line with the hypothesis that Ca2þ selectively promotes single crystal growth. Gd-2 contains an obvious site-occupancy disorder of Cs3, which has been refined on two positions with site occupancies of 0.6 and 0.4. The Tb1 atom in Tb2 exhibits disorder over two positions that were refined with site occupancies of 0.8 and 0.2, respectively, and the Na1 split positions in Tb-2 were described with site occupancies of 0.7 and 0.3. The halfoccupied Cs4 atom in Tb-2 exhibits disorder over two positions that were refined with site occupancies of 0.3 and 0.2. Dy-2 also exhibits disorder, namely, of Na2, on two positions with relative occupancies of 0.6 and 0.4, and the Cl1 atom is disordered into two positions with an occupancy of 0.5. In all of the structures, there is a discrepancy between the formulas determined by elemental analysis and those deduced from the crystallographic atom list. This is due to considerable disorder among the cations and the water molecules, which is a common
phenomenon encountered in POM chemistry. Hydrogen atoms were not included in the refinements. The crystallographic data of all polyanions are summarized in Table 1.
’ RESULTS AND DISCUSSION Synthetic Strategy. We reacted the silicotungstate precursor Na10[A-R-SiW9O34] 3 23H2O ({R-SiW9}) with lanthanide cations (Ln = GdIII, HoIII, TbIII, DyIII) under optimized reaction conditions. Five polymeric polyanions with two frameworkbased structures were successfully isolated in a 1.0 M sodium acetate buffer (pH 4.4) at 80 °C by combining {R-SiW9} and Ln3þ cations in a molar ratio of 1:3 for 90 min. The solution was cooled to room temperature, subsequently filtered off, and set for crystallization. Slow evaporation at room temperature yielded crystals suitable for single-crystal X-ray diffraction, followed by FT-IR and UV/vis spectroscopy, CV and photoluminescence measurements, TGA, and elemental analysis. The polymeric polyanions were isolated as mixed sodium/cesium salts: Na2CsCaGd2[Gd2(H2O)7Si2W18O66]Cl 3 27H2O (Gd-1), Na2.5Cs3.5GdH2[Gd2(H2O)7Si2W18O66](C2H3O2) 3 16H2O (Gd-2), Na2Cs3H2Tb [Tb2(H2O)7Si2W18O66] 3 17H2O (Tb-2), Na4Cs3DyH[Dy2(H2O)6.5(C2H4O2)0.5Si2W18O66]Cl 3 17H2O (Dy-2), and Na4 Cs3Ho[Ho2(H2O)7Si2W18O66] 3 18H2O (Ho-2). Both Gd-1 with a 3D inorganic framework and Gd-2Ho-2 with 2D layer networks are constituted of dimeric building blocks consisting of two [A-R-SiW9O34]10 fragments, which are connected through WOW bonds via two axial oxygen atoms of each individual anion. The WOW bonds are bent toward the interior of the polyanion, thereby forming the pocket of the open WellsDawson ion [R-Si2W18O66]16. The multilacunary polyanions of compounds Gd-1 to Ho-2 have incorporated two lanthanoid cations within their structural cavities to form the 4946
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Figure 1. Transformation of the [A-R-SiW9O34]10 precursor into dimeric [Ln2(H2O)7Si2W18O66]10 [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5(C2H4O2)0.5Si2W18O66]10 polyanions in a HOAc/NaOAc buffer (W, black polyhedra; Si, purple polyhedra; Ln, blue; O, red; C, gray).
dimeric building blocks [Ln2(H2O)7Si2W18O66]10 (Ln = Gd, Ho, Tb) and [Dy2(H2O)6.5(C2H4O2)0.5Si2W18O66]10. These moieties are, furthermore, linked to external lanthanoid atoms via terminal oxygen atoms of the neighboring polyanion (WdO), thereby forming two different framework types (Gd-1 and Gd2Ho-2, respectively; cf. Figure 1). It is noteworthy that previous syntheses of the parent anion were based on potassium salts, which suggests an essential role of Kþ in maintaining the open WellsDawson structure with its special coordination sites for different cations.26,27,29 In the case of the newly formed [Ln2(H2O)7Si2W18O66]10 [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5(C2H4O2)0.5 Si2W18O66]10 polyanions, the lanthanoids occupy the peripheral Kþ position in the [R-Si2W18O66]16 host anion, which was described by Herve et al.26,27 However, we employed a different synthetic strategy toward the lanthanide-containing polyanions starting from the sodium salt of the trivacant Keggin polyoxoanion [A-R-SiW9O34]10 ({R-SiW9}) precursor in a 1.0 M NaOAc buffer throughout in order to suppress the hydrolysis of the lanthanide cations and to adjust the pH of the reaction system. It is well-known that self-assembly processes of lanthanide-substituted POMs are highly affected by reaction parameters such as the pH values, counterions, stoichiometry, temperature, etc.20 Furthermore, the {R-SiW9} polyoxoanion is easily transformed into Keggin- or Dawson-type polyanions and oligomeric structures in an acidic aqueous solution. A literature survey of POM types emerging from the {R-SiW9} precursor can be found in Table S1 in the Supporting Information. The results suggest in their entirety that the {R-SiW9} moiety preferably forms Dawson-type polyanions by dimerization or gives rise to oligomeric structures connected through tungsten atoms or alkali-metal cations at lower pH values (2.4 < pH < 5.9),2631 whereas it is prone to reassembly or isomerization into Keggin-type polyanions at higher pH values (5.0 < pH < 6.3).3537 In the present {R-SiW9}/LnIII systems, the transformation from [R-SiW9O34]10 to [R-Si2W18O66]16 preferably results in the formation of Gd-1 and Gd-2Ho-2 under the given reaction conditions (pH 4.4 and 80 °C). Moreover, the crystal structure of the products is obviously affected by the {RSiW9}/LnIII ratio: the polymeric compounds (Gd-1 to Gd-2)
could not be obtained upon its change from 1:3 to 1:2 or 1:1. The countercation is another important synthetic parameter factor: when Csþ was replaced with NH4þ, Naþ, Kþ, or Rbþ, crystals of sufficient quality for single-crystal X-ray diffraction were difficult to obtain. This may be due to electrostatically superior linker qualities of the larger Csþ in connection with the [Ln2 (H2O)7Si2W18O66]10 [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5(C2H4O2)0.5Si2W18O66]10 polyoxoanions. Most interestingly, Gd-1 with a 3D inorganic framework structure was obtained from self-assembly reactions in a 1.0 M NaOAc buffer solution by adding a small amount of Csþ countercations (0.5 mL of a 1.0 M CsCl solution) to the POM precursor. Continued Csþ addition (1.2 mL) led to transformation of the 3D POM framework compound Gd-1 into the 2D structure of Gd-2 in solution. In addition, a mixture of Gd-1 and Gd-2 in solution could be deliberately produced by adjusting the Csþ concentration, which points to an equilibrium between both compounds. Interestingly, this phenomenon was not observed for Tb-2, Dy-2, or Ho-2, so that the solution equilibria of the new compounds are currently under more detailed investigation. Whereas neither alkali-metal cations nor lanthanoid ions bind to the central pocket site of [Si2W18O66]16, Kþ on this position is obviously essential to maintaining the WellsDawson structure of [{K(H2O)3}2{K(H2O)2}(Si2W18O66)]13.26,27 It goes without saying that the templating role of the cations during POM formation processes cannot be underestimated, as we have, for example, observed for Csþ as a stabilizator of the [Cs⊂Ln6As6W63O218(H2O)14(OH)4]25 (Ln = Eu, Gd, Tb, Dy, Ho, Er) series.16a Although Herve et al. pointed out that dimerization of [NaSi2W18O66]15 cannot be ruled out, their attempt to study the influence of Naþ on the reactivity of [A-RSiW9O34]10 led to the formation of monolacunary [A-RSiW11O39]8, which indicates that the affinity of Kþ for the central position is caused by the size and solubility differences compared to Naþ. Crystal Structures. Although compounds Gd-1, Tb-2, Dy-2, Ho-2, and Gd-2 have the same dimeric building block in common, the polymeric structure of Gd-1 differs from the Gd2Ho-2 series, as can be seen from the crystallographic data (cf. Table 1). Generally, two lanthanoid cations formally replace 4947
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Figure 2. (a) Connectivity of the {Gd2[Gd2(H2O)7Si2W18O66]}4 anion in Gd-1 (W, blue; Gd, green; Si, yellow; O, red). Individual Gd geometries of Gd-1: (b) tricapped trigonal-prismatic coordination of Gd1; (c) dodecahedral geometry of Gd2; (d) monocapped squareantiprismatic environment of Gd3.
the potassium cations on the exterior pocket sites of the open WellsDawson parent type26 [{K(H2O)3}2{K(H2O)2}(Si2W18 O66)]13. The remaining lanthanoid cations are external linkers, thus leading to the formation of 3D networks (Gd-1) or 2D polymeric sheetlike materials (Gd-2, Tb-2, Dy-2, and Ho-2). The solid-state structure of Gd-1 (Figures 2 and 3) consists of the association of one WellsDawson anion A-R-[Si2W18O66]16 with four Gd3þ cations: the Gd1 and Gd2 cations are located in the peripheral pocket of the R-[Si2W18O66]16 anion, whereas the Gd3 and Gd4 cations occupying the R-[Si2W18O66]16 moiety are bound to the terminal oxygen atoms of the tungsten caps contributed by the monomeric [A-R-SiW9O34]10 precursor. The GdGd distance is 6.338(2) Å in the dimeric WellsDawson anion [Gd2(H2O)7Si2W18O66]10 of Gd-1. The Gd1 cation is bound to four terminal oxygen atoms (O20, O21, O26, and O27) from pairs of edge-sharing WO6 octahedra of the R-[Si2 W18O66]16 framework [Gd1O distance range: 2.372(9) 2.538(9) Å], to four terminal water ligands (O50, O51, O52, and O53) [Gd1O distances: 2.438(11)2.475(11) Å], and to a terminal oxygen atom (O15T0 , symmetry code 1 x, y, 0.5 z) from another neighboring [Gd2(H2O)7Si2W18O66]10 moiety [Gd1O15T0 : 2.494(10) Å]. The Gd2 cation is also bound to four terminal oxygen atoms (O22, O23, O28, and O29) from pairs of edge-sharing WO6 octahedra [Gd2O distances: 2.338(9)2.418(10) Å] and to three water molecules [O54, O55, and O56 with Gd2O ranging from 2.405(13) to 2.456(10) Å]. Gd2 is, furthermore, connected to a terminal oxygen atom (O6T0 ; symmetry code 1 x, y, z) from a neighboring polyanion [Gd2O6T0 : 2.407(9) Å] via symmetry-related GdOW bonds (Gd2O6T0 W60 and Gd20 O6TW6), with an inversion center displaying a head-on coordination motif including four metal atoms in the dimeric entity [Gd2(H2O)7Si2W18O66]10 (Figure 2a).
Figure 3. Packing motif of the Gd-1 type. The cations and crystal water molecules are omitted for clarity (W, blue octahedra; O, red; Si, yellow; Ln, green): (a) polyhedral view of the 3D open framework with 1D channels in Gd-1; (b) projection along the y axis.
In contrast, the Gd1 cation of the dimer is coordinated to the terminal oxygen atom of W15, thus connecting six metal centers into a hexameric arrangement with inversion symmetry. Of the two Gd3 and Gd4 cations coordinated to the terminal oxygen atoms of the dimeric polyanion [Gd2(H2O)7Si2W18O66]10, Gd3 is coordinated to W4, W10 (1 x, y, 0.5 z), and W18 (0.5 þ x, 0.5 þ y, z) and vice versa via μ-oxo bonds [Gd3O: 2.366(10)2.422(9) Å]. Gd4 is coordinated to W1 (0.5 x, 0.5 y, z) and W12 of the open WellsDawson anion via μ-oxo bonds [Gd4O1T0 , 2.319(11) Å; Gd4O12T, 2.316(10) Å], again in a symmetry-related fashion with an inversion center. The Gd3 coordination sphere is completed by six water molecules, whereas the Gd4 environment is occupied by seven water molecules. While Gd1, Gd2, and Gd4 are coordinated to two polyanions, Gd3 displays the highest degree of connectivity, being attached to three clusters. Therefore, each dimeric cluster [Gd2(H2O)7Si2W18O66]10 is further linked into a 3D polymeric material via four gadolinium cations (cf. Figure 3). It is noteworthy that this connection mode results in the formation of 1D channels with incorporated crystal water molecules and alkalimetal cations. The cross section of the channels is about 12.7 7.1 Å2. From the topological point of view, Gd1 and Gd2 can be assigned as the bridging connectors between two [Gd2 (H2O)7Si2W18O66]10 clusters. Consequently, [Gd2(H2O)7Si2 W18O66]10 clusters, Gd3 and Gd4, can be considered as the nodes. In this stylized manner, [Gd2(H2O)7Si2W18O66]10 moieties are 7-connecting nodes, Gd3 atoms are 3-connecting nodes, and Gd4 atoms are 2-connecting nodes. Therefore, the 4948
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Figure 4. View of the topology of Gd-1 (red nodes, [Gd2(H2O)7Si2W18 O66]10 clusters; green nodes, Gd3 atoms; blue nodes, Gd4 atoms).
Figure 6. Packing motif of the Tb-2 type. The cations and crystal water molecules are omitted for clarity (W, blue; O, red; Si, yellow; Ln, green): (a) polyhedral view of 1D chains in the xz plane; (b) 2D sheet projection along the x axis.
Figure 5. (a) Ball-and-stick representation of the {Tb[Tb2(H2O)7 Si2W18O66]}7 anion in Tb-2 (W, blue; Tb, green; Si, yellow; O, red). (b) Dodecahedral coordination environment of Tb1A in Tb-2. Only the major position of the disordered Tb1 (Tb1A) is shown for clarity.
3D framework can be described as a 3,7-connecting network with the Schl€afli symbol [(3.62)(32.68.72.84.95; Figure 4]. To the best of our knowledge, Gd-1 represents the first 3D inorganic coordination polymer based on lanthanoid-substituted WellsDawson POMs, and the topology of this framework has never been observed in POM chemistry before. Gd-2, Tb-2, Dy-2, and Ho-2 all have the triclinic space group P1 in common, and their molecular structures are composed of one WellsDawson anion A-R-[Si2W18O66]16 and three crystallographically different lanthanoid cations (Ln = Tb, Dy, Ho, Gd). Because the four compounds are isomorphous, the structure of Tb-2 is described in detail as a representative example. In the Tb-2 polyanions, the Tb1 and Tb2 cations occupy the pocket positions of the [Si2W18O66]16 host anion with a TbTb distance of 6.265(2) Å (Figure 5a). The Tb1A cation is bound to four terminal oxygen atoms (O22, O23, O28, and O29) from pairs of edge-sharing WO6 octahedra of the R-[Si2W18O66]16 framework [Tb1AO distances: 2.317(11)2.411(10) Å] and to four terminal water ligands [O51, O52, O53, and O73; Tb1AO distances between 2.36(2) and 2.459(14) Å].
The Tb2 cation, on the other hand, is not only attached to four terminal oxygen atoms (O20, O21, O26, and O27) from the R-[Si2W18O66]16 framework [Tb2O distances: 2.292(10)2.398(10) Å] and three terminal water ligands [O49, O50, and O69; Tb2O distances between 2.387(11) and 2.472(12) Å] but also bridged to another single polyanion, which is connected to the adjacent cluster via symmetry-related TbOW bonds [Tb2O6T0 W60 and Tb20 O6TW6; the symmetry code of O6T0 , W60 , and Tb20 is 1 x, y, 2 z with a Tb2O6T0 distance of 2.341(9) Å], thereby forming a similar head-on species of four metal centers via an inversion center, as has been observed in Gd-1 (Figure 5a). The Tb3 cations are coordinated to three terminal oxygen atoms, O4T, O18T0 (symmetry code x, 1 þ y, z), and O17T0 (symmetry code x, y, 1 z), of the dimeric [Tb2(H2O)7 Si2W18O66]10 polyanions [Tb3O: 2.321(11)2.371(10) Å] and to five water molecules [O55O59 with Tb3O distances ranging from 2.383(13) to 2.425(12) Å]. Tb3 is attached to three clusters through W4, W18 (x, 1 þ y, z), and W17 (x, y, 1 z) via μ-oxo bridges, thus connecting the 1D polyanion chains into a 2D sheetlike polymeric material with voids for alkali-metal cations and crystal water molecules (Figure 6). From the topological point of view, the [Tb2(H2O)7Si2 W18O66]10 clusters represent 4-connecting nodes, the Tb2 atoms can be assigned as bridging connector ligands between two clusters, and the Tb3 atoms are also representing 3-connecting nodes (Figure 7). Therefore, the Schl€afli symbol for this 3,4-connected binodal network is (42.6)(42.62.82). Moreover, it should be noted that there are some slight structural differences 4949
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Figure 7. Topological view of Tb-2 along the x axis (red nodes, [Tb2(H2O)7Si2W18O66]10 clusters; green nodes, Tb3 atoms).
among Tb-2, Dy-2, Ho-2, and Gd-2: whereas a half-occupied acetate oxygen and a half-occupied water molecule are bound to the Dy1 ion in Dy-2, the analogous bonding sites of the Ln1 ions in Tb-2 and Ho-2 are occupied by one terminal water molecule (Figure 1). Furthermore, the LnIII cations in Tb-2, Dy-2, and Ho2 are eight-coordinate, with an almost undistorted dodecahedral coordination environment (Figure 5). In Gd-2, the Gd1 and Gd2 cations, located in the external pocket of the R-[Si2W18O66]16 anion, are eight-coordinate, with a nearly ideal dodecahedral coordination and a distorted square-antiprismatic coordination, respectively. Gd3 is nine-coordinate, adopting a distorted ninecoordinated monocapped square antiprism, with three terminal oxygen atoms from three neighboring [Gd2(H2O)7Si2 W18O66]10 polyanions and four terminal water molecules. The remaining two coordination sites are occupied by two oxygen atoms of the bidentate acetate ligand (cf. Figure 8 and discussion below). All polyanions are arranged as “inversion pairs” in analogy to K16-R-[Si2W18O66].22 However, the lanthanoid cations occupy the exterior pockets of the open WellsDawson R-[Si2W18 O66]16 anion, and they act as external linkers, thereby differing from the role of Kþ in previous structures and leading to the formation of novel polymeric motifs. It is noteworthy that the trivalent lanthanoid ions usually exhibit variable higher coordination numbers: eight (dodecahedral, square antiprismatic, or bicapped trigonal prismatic) and nine (tricapped trigonal prismatic or monocapped square antiprismatic).38 Coordination environments of comparable extension have also been described for cerium-containing polyoxotungstates, such as those for {Ce16W148} with two, five, or no aqua ligands per cerium atom17 and those for {Ce20W100} with one or two aqua ligands.18 The same trend applies for our recently reported gadolinium-containing polyoxotungstate {Gd8W124}.16b The lanthanoid ions in the present series (Gd1Ho-2) exhibit four different coordination geometries with three to seven terminal aqua ligands, respectively. Concerning Gd-1, the coordination polyhedron of Gd1 can be described as a nine-coordinated tricapped trigonal prism (D3h), with the capping oxygen atoms located in the center of three rectangular faces (Figure 2b). The trigonal faces of the tricapped trigonal prism are
Figure 8. (a) Ball-and-stick representation of the Gd[Gd2(H2O)7Si2W18 O66]}7 anion in Gd-2 (W, blue; Tb, green; Si, yellow; O, red; C, gray). Individual Gd geometries of Gd-2: (b) dodecahedral coordination environment of Gd1; (c) square-antiprismatic geometry of Gd2; (d) monocapped square-antiprismatic environment of Gd3 in Gd-2.
defined by O50O26O20 and O52O51O53, with O50 eclipsing O52, O26 eclipsing O51, and O20 eclipsing O53. Three oxygen atoms (O21, O27, and O15T) as the three capping atoms of the rectangular faces are approximately trigonal coplanar, with an average angle between capping oxygen atoms and Gd1 of 119.9(2)°, in comparison to 120° for an ideal tricapped trigonal prism. The dihedral angles between the plane defined by the capping atoms and Gd1 and the two trigonal planes are 1.0(4)° and 0.9(3)°, respectively, and the dihedral angle between the two trigonal planes is 1.5(4)°, thereby rendering the overall geometry close to an ideal tricapped trigonal prism.39 Bond angles between Gd1 and two eclipsing oxygen atoms of opposite trigonal planes are 90.8(4)° for O50Gd1O52, 90.7(4)° for O26Gd1O51, and 92.6(4)° for O20Gd1O53. The coordination geometry around Gd2 is best described as an eight-coordinated dodecahedron (Figure 2c) with an idealized D2d symmetry based on the visualization of two interpenetrating trapezoids that are orthogonal to each other.40 In the case of Gd2, these trapezoids are defined as the near-planar arrangements of O54O56O55O6T and O22O23O29O28 with average deviations from their leastsquares planes of 0.7938 and 0.0212 Å, respectively. The dihedral angle between the two trapezoids is found to be 89.4(2)°. The coordination geometries of both Gd3 and Gd4 are quite close to monocapped square antiprisms with idealized C4v symmetry. In the case of Gd3, for example (Figure 2d), the two approximately antiparallel squares are constituted of O61O62O60O59 and O58O4TO57O10T with a dihedral angle of 2.9(3)°.41 The capping atom (O18T) is located above the open square plane of O61O62O60O59. The according base diagonals are 3.693(2) and 4.113(2) Å for O4TO10T and O57O58, 4950
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry respectively. They are somewhat different owing to the longer distances of 3.012(2) Å for O57O10T and 2.712(2) Å for O4TO57, compared to the other two distances in the square, 2.640(2) and 2.703(2) Å for O4TO58 and O58O10T, respectively. Although both Gd1 and Gd2 in Gd-2 are eight-coordinate, their local geometries can be differentiated into an almost ideal dodecahedron (D2d) and a slightly distorted square antiprism (D4d), respectively (Figure 8b,d). In the case of the Gd1 cation, two body diagonals of the trapezoids are defined as O74O73O72O71 and O38O37O29O30. The dihedral angle between the trapezoids is 88.8(2)°. In the case of Gd2, two groups of oxygen atoms, namely, (O33, O35, O41, and O69) and (O34, O70, O36, and O68), constitute the two bottom planes of a square antiprism, and the average deviations from their least-squares planes are 0.1119 and 0.1096 Å, respectively. The dihedral angle for the two bottom planes is 5.1(2)°. The Gd3 cation is located in a distorted monocapped square antiprism (Figure 8c), with O78 from one acetate ligand in the capping position. The two antiparallel squares are constituted of O77O6O79O84 and O76O2O75O45, with average deviations of 0.2410 and 0.1527 Å, respectively. The dihedral angle between the two bottom squares is 6.2(3)°. For Tb-2, Dy-2, and Ho-2, the coordination environment of all of the lanthanoids can be described as an almost undistorted eightcoordinated dodecahedron (D2d). Figure 5b displays a nearperfect dodecahedral coordination geometry around the Tb1 cation as a representative example, with the dihedral angle between the two trapezoids being 88.9(2)°. These results show that larger lanthanoids prefer higher coordination numbers and display more flexible coordination geometries compared to smaller lanthanoids: the electrostatic stability of the crystal structure decreases with the lanthanoid radius because of the increasing ligand repulsion in the coordination sphere.42 Bond-valence-sum calculations43 revealed that the valencies of all metal and oxygen atoms within the polyanions [Ln2(H2O)7 Si2W18O66]n10n [Ln = GdIII (Gd-1 and Gd-2), TbIII, HoIII] and [Dy2(H2O)6.5(C2H4O2)0.5Si2W18O66]n10n are in agreement with their intracluster bonds so that none of the oxygen atoms of the dimeric {R-Si2W18O66} moiety is protonated. Seven or 6.5 terminal aqua ligands, respectively, are coordinated to two of the lanthanoid ions located in the external pocket of the open WellsDawson anion {R-Si2W18O66}. This sums up to a net charge of 10 for the above-mentioned polyanions, which is compensated for by their countercations in the solid state. However, to balance the charge, we added two protons in Tb-2, one proton in Dy-2, and two protons in Gd-2, respectively, as the products were isolated from an acidic aqueous solution (pH 4.4). These protons cannot be located crystallographically and are assumed to be delocalized over the entire structure, which is a commonly observed phenomenon in the chemistry of POMs.44 Moreover, the average LnO distances in all of the compounds tentatively indicate the presence of a lanthanoid contraction effect with 2.42(2) Å for Gd-1, 2.41(1) Å for Gd-2, 2.39(3) Å for Tb-2, 2.36(2) Å for Dy-2, and 2.34(2) Å for Ho-2. FT-IR Spectroscopy. The FT-IR spectra of all compounds (Gd-1 and Gd-2, Tb-2, Dy-2, and Ho-2) display related characteristic νas(SiOa), terminal νas(WOt), corner-sharing νas(WOb), and edge-sharing νas(WOc) asymmetrical vibration peaks due to the presence of the common open WellsDawson anion A-R-[Si2W18O66]16 (cf. Figure S1 in the Supporting Information).1 In the IR spectrum of Gd-1, the peak at
ARTICLE
1001 cm1 can be attributed to νas(SiOa) and the characteristic bands at 938, 871, 833, 808, and 723 cm1 are assigned to νas(WOt), νas(WOb), and νas(WOc). The characteristic features in the IR spectrum of Gd-2 at 1002, 934, 886, 814, and 720 cm1 arise from νas(SiOa), νas(WdOd), νas(WOb), and νas(WOc), respectively. The peaks in the IR spectrum of Tb-2 at 1002, 937, 876, 818, and 718 cm1 can be assigned to νas(SiOa), νas(WdOd), νas(WOb), and νas(WOc). In the IR spectrum of Dy-2, the peaks at 1002, 940, 882, 817, and 716 cm1 are attributed as follows: νas(SiOa), νas(WdOd), νas(WOb), and νas(WOc). Likewise, the characteristic vibrations in the IR spectrum of Ho-2 at 1003, 939, 868, 833, 809, and 714 cm1 arise from νas(SiOa), νas(WdOd), νas(WOb), and νas(WOc). Moreover, the gradual blue shift of the νas(WOc) vibration points to the influence of the lanthanoid contraction on the FT-IR spectra. UV/Vis Spectroscopy. UV/vis spectra of Gd-1 and Gd-2, Tb-2, Dy-2, and Ho-2 were recorded in an aqueous solution in the 600190 nm range (cf. Figure S2 in the Supporting Information). The UV spectra of Gd-1 and Tb-2 have two characteristic absorption bands at 202205 and 250 nm in common. The absorption band at higher energies can be ascribed to the pπdπ charge-transfer transitions of the Ot f W bonds, whereas the latter low-energy absorption band is due to the pπdπ charge-transfer transitions of the Ob(c) f W bonds. However, the UV spectra of Gd-2, Dy-2, and Ho-2 display only the higher-energy absorption band centered at 194200 nm that can be assigned to the pπdπ charge-transfer transitions of the Ot f W bonds.45a The blue shift of the absorption bands at higher energies might reflect the influence of the different lanthanide cations on the local geometry of the dimeric [Ln2(H2O)7Si2W18O66]10 (Ln = Gd, Ho, Tb) and [Dy2 (H2O)6.5(C2H4O2)0.5Si2W18O66]10 polyanions. Similar phenomena had already been reported in previous related studies on the reaction of lanthanide cations with monovacant Keggin polyoxotungstates.45 However, we did not observe the absorption bands of the trivalent lanthanides in an aqueous solution, which may be due to concealment by the strong (O f W) charge-transfer bands. Therefore, we also recorded the solid-state absorption spectra of all samples in the 400850 nm range. For Tb-2, two weak absorption bands around 466 and 498 nm correspond to the 7F6 f 5D3 and 7F6 f 5D4 transitions of the Tb3þ ion (cf. Figure S3 in the Supporting Information). Three weak absorption bands appear in the visible range for Dy-2 at 428, 453, and 475 nm, and they are assigned to the 6H15/2 f 4 F9/2, 6H15/2 f 4I15/2, 6H15/2 f 4G11/2 transitions of Dy3þ. Two stronger bands at 757 and 806 nm in the near-IR region indicate the 6H15/2 f 6F3/2 and 6H15/2 f 6F5/2 transitions of the Dy3þ ion, respectively (cf. Figure S4 in the Supporting Information).46 For Ho-2, seven absorption bands around 418, 451, 468, 474, 486, 537, and 642 nm can be assigned to the 5I8 f 5G5, 5I8 f (5F1, 5G6), 5I8 f 3K8, 5I8 f 5F2, 5I8 f 5F3, 5I8 f (5F4, 5S2), and 5 I8 f 5F5 transitions of the Ho3þ ion (Figure 9), but only the 5I8 f (5F1, 5G6) and 5I8 f (5F4, 5S2) transitions notably contribute to the color of this compound.47 Interestingly, there is a rapid color change between light yellow and pink when the Ho-2 sample is illuminated with incandescent light or daylight because of the light-source-dependent color of the Ho3þ centers.46 This is a promising feature for the preparation of photochromic inorganic materials.47 PXRD Characterization. The phase purity of representative Gd-1 and Gd-2, Tb-2, Dy-2, and Ho-2 samples was checked by 4951
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Figure 9. Solid-state UV/vis spectra of Ho-2 measured in the 300700 nm range. Inset: color change of Ho-2 upon irradiation from different light sources.
bulk PXRD measurements (Figures S10S14 in the Supporting Information). The PXRD patterns for the Gd-2Ho-2 series are quite similar, indicating the isostructural character of the four compounds. The experimental diffraction patterns are in line with the calculated data, thus confirming the results of singlecrystal X-ray structure determination. Photoluminescence Spectroscopy. In order to investigate the photoluminescence behavior of Gd-1 and Gd-2, Tb-2, Dy-2, and Ho-2, their spectra were recorded at room temperature upon photoexcitation. Only Tb-2 and Dy-2 exhibit millisecondorder luminescence lifetimes that could be measured under the given conditions (Figure 10). The terbium compound Tb-2 exhibited green photoluminescence under excitation at 255 nm. The emission spectrum displays four characteristic emission peaks of Tb3þ at 487, 532, 579, and 624 nm, which can be assigned to transition of the 5D4 excited state to the corresponding ground state 7FJ (J = 6, 5, 4, 3) of the Tb3þ ion.48 The 5 D4 f 7F6 transition is a magnetic-dipole transition, and its intensity varies with the strength of the ligand field experienced by the Tb3þ ion. The emission to magnetic-dipole transition (5D4 f 7F6) in Tb-2 does not show splitting, which is in agreement with the results of the crystal structure determination that indicate closely related coordination environments for the terbium ions. The strongest emission band 5D4 f 7F5 is an electric-dipole transition that is exceptionally sensitive to changes in the chemical bonds in the vicinity of the Tb3þ ion. The intensity of the 5D4 f 7F5 transition increases with a decrease in the site symmetry of the Tb3þ ion. Therefore, the intensity ratio of the I(5D4f7F5) to I(5D4f7F6) transitions is frequently used to quantify the coordination state and site symmetry of the rare-earth ions.48 In the present case, the intensity ratio I(5D4f7F5) to I(5D4f7F6) is about 3.1, which further confirms the closely related low-symmetry coordination environments of the three Tb3þ ions. The dysprosium-containing POM Dy-2 displays two characteristic 4F9/2 f 6H15/2 and 4 F9/2 f 6H13/2 transitions upon excitation at 350 nm, leading to blue (around 479 nm) and yellow (around 574 nm) emission, respectively.49 The 4F9/2 f 6H13/2 transition is assigned to a hypersensitive transition with ΔJ = 2, which is strongly influenced by the chemical environment of Dy3þ. Generally, the low intensity of the luminescence of the Dy3þ ion in complexes can be explained in terms of effective radiationless
Figure 10. Photoluminescence spectra of Tb-2 (a) and Dy-2 (b) at room temperature (excitation wavelengths at 255 and 350 nm).
deactivation in the excited state due to the small energy gap between the excited level 4F9/2 and the sublevels of the groundstate terms 6H3/2, 6H5/2, and 6H5/2.50 Magnetic Properties. The magnetic susceptibility of Gd-1 and Gd-2 was investigated with respect to the magnetic Gd3þ centers. Plots of the molar magnetic susceptibility χm per gadolinium ion and 1/χm vs T in the range between 2 and 300 K for an applied magnetic field of 2000 Oe are shown in Figure 11. Both Gd-1 and Gd-2 display characteristic paramagnetic behavior over the entire temperature range, and the experimental data fit well to a Curie law (χ = C/T) with the respective Curie constants of CGd-1 = 8.00 emu K Oe1 mol1 and CGd-2 = 8.20 K Oe1 mol1. Likewise, the 1/χm vs T curves are almost perfectly linear. The effective magnetic moments μeff per gadolinium ion [μeff2 = 3Ck/μB2N (k = Boltzmann's constant, μB = Bohr magneton, and N = Avogadro’s number)] were derived from the Curie constant. The obtained values of 8.03 μB for Gd-1 and 8.13 μB for Gd-2 are close to the expected spin-only value (μeff = 7.94 μB) for the free Gd3þ ion. Furthermore, the refined spin values S for Gd-1 and Gd-2 were determined as 3.54 and 3.58, respectively, which agrees well with the spin of noninteracting gadolinium centers (S = 7/2). These results also indicate that a spinspin coupling through OWO bridges is negligible because of large GdGd distances in both Gd-1 and 4952
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry
ARTICLE
Figure 12. Cyclic voltammograms of 0.2 mM Gd-1 in a pH 4.4 (1.0 M CH3COONa/CH3COOH) buffer at different scan rates (from inner to outer plots: 100, 120, 140, 160, 180, 200, 220, 240, 260, and 300 mV s1). Inset: plots of the anodic and cathodic peak currents of II0 against the scan rates.
Figure 11. Temperature dependence of the magnetic susceptibility χm and χm1 (inset) from 2 to 300 K for (a) Gd-1 and (b) Gd-2.
Gd-2. We observed related phenomena in our previous studies on other gadolinium-containing POMs.16 Electrochemistry. In order to electrochemically characterize compounds Gd-1 and Gd-2Ho-2, we carried out CV measurements in a sodium acetate buffer (pH 4.4) solution as the supporting electrolyte (Figure 12). The results indicate that all compounds show almost identical CV behavior, which is probably because of the common presence of the WellsDawson anion A-R-[Si2W18O66]16 in their structures. For example, the reduction waves of Gd-1 occur at 0.657 V (Epc1) and 0.901 V (Epc2), respectively, in two separate steps. These waves can be assigned to the reduction of tungsten centers. During the reoxidation process, one oxidation peak Epa1 located at 0.562 V is associated with first reduction wave Epc1. The peak potential difference between Epa1 and Epc1 is 95 mV for this redox couple (II0 ), corresponding to a reversible one-electron-redox process.51 However, the reoxidation wave associated with the second reduction process is more complex through the splitting of the reoxidation pattern of tungsten waves into two waves located at 0.806 V (Epa2) and 0.682 V (Epa3). Related observations have been encountered in the electrochemical behavior of dilacunary [γ-SiW10O36]8 and the transition-metal-substituted decatungstosilicate [M(H2O)2(γ-Si2W20O70)]10 (M = Mn2þ, Co2þ, Ni2þ).31,32 These results might indicate that a
strong irreversible electron-transfer process takes place in the second redox step. Furthermore, no redox activity of lanthanide cations was detected over the potential range from 1.0 to þ1.0 V, which is in line with studies on the redox processes of lanthanide-substituted Dawson-type arsenotungstates (R2-[Ln(As2W17O61)2]17 and {[(R2-As2W17O61)Ln(H2O)2]2}14).52 The CV curves of Gd-1 at different scan rates were also investigated. When the scan rate was changed from 100 to 300 mV s1, the peak potentials varied gradually: the cathodic peak potentials were shifted toward negative values, whereas the corresponding anodic peak potentials were shifted to the opposite direction with an increase of the scan rate. In addition, the peak currents are proportional to the scan rate (ν), which indicates that the redox process is surface-controlled with a fast exchange rate of electrons. Because the cyclic voltammograms of Tb-2, Dy-2, Ho-2, and Gd-2 exhibit almost identical CV curves in comparison with Gd-1 (Figures S6S9 in the Supporting Information), they are not individually discussed. TGA. TGA measurements on Gd-1 and Gd-2, Tb-2, Dy-2, and Ho-2 were performed under a nitrogen flow in the temperature range from 30 to 800 °C. The TGA curves of all of the compounds (shown in Figure S5 in the Supporting Information) exhibit one weight loss step in the temperature range of 30300 °C, respectively. The observed weight loss for Gd-1 is 10.3% (calcd 10.2%), corresponding to the release of crystal water molecules and adsorbed water molecules. The corresponding values are 5.2% (calcd 5.3%) for Tb-2 and 6.7% (calcd 7.6%) for Ho-2. For Dy-2, one weight loss step of 7.6% corresponds to the loss of water molecules and 0.5 formula units of the acetate ligand (calcd 7.9%). For Gd-2, one weight loss stage of 7.8% (calcd 7.9%) can be assigned to the loss of water molecules and one acetate ligand. The related shapes of the TGA curves, furthermore, underscore the structural similarities of the compounds.
’ CONCLUSIONS A series of five lanthanoid-containing silicotungstates of the novel [Ln2(H2O)7Si2W18O66]10 (Ln = Gd, Ho, Tb) and [Dy2 (H2O)6.5(C2H4O2)0.5Si2W18O66]n10n types were obtained 4953
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry from the one-step reaction of the [A-R-SiW9O34]10 precursor with LnIII cations in buffer solutions. All compounds were structurally characterized, and their packing motifs depend on the size of the lanthanoid cation. Whereas the Gd-1 representative of the new compound family crystallizes in a 3D network structure, Gd-2 and the remaining compounds consist of 2D polyoxotungstate sheets. This is in line with the special role of Gd3þ in our previous studies on large polyoxotungstates, because the novel {Gd8W124} type is exclusively formed with this member of the lanthanoid series.16b The individual coordination environments of the lanthanoid cations also differ between the two new 3D and 2D compound types. Both structural motifs display accessible voids that are occupied by alkali-metal cations and crystal water molecules. The influence of the lanthanoid contraction is also evident from the FT-IR spectra, and the newly discovered family of open WellsDawson host anions with lanthanoid guests was characterized with a wide range of analytical methods. Their electrochemical properties were studied by CV in a sodium acetate buffer (pH 4.4) as the supporting electrolyte. The Tb-2 and Dy-2 compounds exhibit room temperature photoluminescence upon excitation, and the Ho-2 compound displays photochromic behavior. The magnetic behavior of Gd-1 and Gd-2 between 2 and 300 K was found to be paramagnetic and in agreement with the spin of noninteracting gadolinium centers. In conclusion, our work provides new incentives to explore controllable assemblies and structural transformations of Ln-POM-based coordination polymers with distinct structural features and properties.
’ ASSOCIATED CONTENT Supporting Information. X-ray crystallographic files (in CIF format), product range emerging from the [A-RSiW9O34]10 precursor, FT-IR spectra, UV/vis spectra, TGA, cyclic voltammograms, and PXRD patterns for compounds Gd-1, Tb-2, Dy-2, Ho-2, and Gd-2. This material is available free of charge via the Internet at http://pubs.acs.org.
bS
’ AUTHOR INFORMATION Corresponding Author
*E-mail:
[email protected]. Tel: þ41 44 635 4691. Fax: þ41 44 635 6802.
’ ACKNOWLEDGMENT This work was supported by the Swiss National Science Foundation (SNSF Professorship PP002-114711/1), and financial support from the University of Zurich is gratefully acknowledged. The authors thank Prof. Dr. Markus Niederberger, Dr. Marta D. Rossell, and Niklaus Kr€anzlin (Laboratory for Multifunctional Materials, Department of Materials, ETH Zurich) for PXRD measurements. L.N. thanks the China Scholarship Council for a Ph.D. research fellowship. ’ REFERENCES (1) Pope, M. T. Heteropoly and Isopoly Oxometalates; Springer: Berlin, 1983. (2) Pope, M. T.; M€uller, A. Angew. Chem. 1991, 103, 56. Angew. Chem., Int. Ed. 1991, 30, 34–48. (3) Pope, M. T. Compr. Coord. Chem. II 2003, 4, 635–678.
ARTICLE
(4) Hill, C. L. Compr. Coord. Chem. II 2003, 4, 679–759. Hill, C. L.; Prosser-McCartha, C. M. Coord. Chem. Rev. 1995, 143, 407–455. (5) Cronin, L. Compr. Coord. Chem. II 2003, 7, 1–56. (6) Polyoxometalate Molecular Science; Borras-Almenar, J. J., Coronado, E., M€uller, A., Pope, M. T., Eds.; Kluwer: Dordrecht, The Netherlands, 2004. (7) Polyoxometalates: From Platonic Solids to Antiretroviral Activity; Pope, M. T., M€uller, A., Eds.; Kluwer: Dordrecht, The Netherlands, 1994. (8) Kortz, U.; M€uller, A.; van Slageren, J.; Schnack, J.; Dalal, N. S.; Dressel, M. Coord. Chem. Rev. 2009, 253, 2315–2320. (9) K€ogerler, P.; Tsukerblat, B.; M€uller, A. Dalton Trans. 2010, 39, 21–36. (10) Hill, C. L. Ed. Chem. Rev. 1998, 98, 1389 (Special Issue on Polyoxometalates). (11) (a) Hasenknopf, B. Front. Biosci. 2005, 10, 275–287. (b) Korenev, V. S.; Boulay, A. G.; Dolbecq, A.; Sokolov, M. N.; Hijazi, A.; Floquet, S.; Fedin, V. P.; Cadot, E. Inorg. Chem. 2010, 49, 9740–9742. (c) Orlandi, M.; Argazzi, R.; Sartorel, A.; Carraro, M.; Scorrano, G.; Bonchio, M.; Scandola, F. Chem. Commun. 2010, 46, 3152–3154. (d) Yin, Q.; Tan, J. M.; Besson, C.; Geletii, Y. V.; Musaev, D. G.; Kuznetsov, A.; Luo, Z.; Hardcastle, K. I.; Hill, C. L. Science 2010, 328, 342–345. (12) Polyoxometalate Chemistry: From Topology via Self-Assembly to Applications; Pope, M. T., M€uller, A., Eds.; Kluwer: Dordrecht, The Netherlands, 2001. (13) Katsoulis, D. E. Chem. Rev. 1998, 98, 359–387. (14) (a) Howell, R. C.; Perez, F. G.; Jain, S. W.; Horrocks, D., Jr.; Rheingold, A. L.; Francesconi, L. C. Angew. Chem., Int. Ed. 2001, 40, 4031–4034. (b) Yamase, T.; Naruke, H.; Sasaki, Y. J. Chem. Soc., Dalton Trans. 1990, 1687–1696. (c) Niu, J. Y.; Guo, D. J.; Wang, J. P.; Zhao, J. W. Cryst. Growth Des. 2004, 4, 241–247. (d) Niu, J. Y.; Wei, M. L.; Wang, J. P.; Dang, D. B. Eur. J. Inorg. Chem. 2004, 160–170. (e) Mialane, P.; Dolbecq, A.; Secheresse, F. Chem. Commun. 2006, 3477–3485. (f) Zhongfeng, L.; Weisheng, L.; Xiaojing, L.; Fengkui, P.; Yingxia, L.; Hao, L. Magn. Reson. Imaging 2007, 25, 412–417. (15) (a) Hussain, F.; Spingler, B.; Conrad, F.; Speldrich, M.; K€ ogerler, P.; Boskovic, C.; Patzke, G. R. Dalton Trans. 2009, 4223–4225. (b) Hussain, F.; Conrad, F.; Patzke, G. R. Angew. Chem. 2009, 121, 9252– 9255. Angew. Chem., Int. Ed. 2009, 48, 9088–9091. (c) Hussain, F.; Patzke, G. R. CrystEngComm 2011, 13, 530–536. (16) Wassermann, K.; Dickman, M. H.; Pope, M. T. Angew. Chem. 1997, 109, 1513–1516. Angew. Chem., Int. Ed. 1997, 36, 1445–1448. (17) Bassil, B. S.; Dickman, M. H.; R€omer, I.; von der Kammer, B.; Kortz, U. Angew. Chem., Int. Ed. 2007, 46, 6192–6195. (18) Hussain, F.; Gable, R. W.; Speldrich, M.; K€ogerler, P.; Boskovic, C. Chem. Commun. 2009, 328–330. (19) (a) Pope, M. T. Handbook on the Physics and Chemistry of Rare Earths; North-Holland: Amsterdam, The Netherlands, 2007; Vol. 38, pp 337382. (b) Drewes, D.; Piepenbrink, M.; Krebs, B. Z. Anorg. Allg. Chem. 2006, 632, 534–536. (c) Li, F.; Xu, L.; Wei, Y.; Gao, G.; Fan, L.; Li, Z. Inorg. Chim. Acta 2006, 359, 3795–3799. (d) Mialane, P.; Dolbecq, A.; Marrot, J.; Secheresse, F. Inorg. Chem. Commun. 2005, 8, 740–742. (e) Fang, X.; Anderson, T.; Benelli, C.; Hill, C. L. Chem.—Eur. J. 2005, 11, 712–718. (f) Fukaya, K.; Yamase, T. Angew. Chem., Int. Ed. 2003, 42, 654–658. (g) Xue, G. L.; Vaissermann, J.; Gouzerh, P. J. Cluster Sci. 2002, 13, 409–421. (h) Cronin, L.; Beuggholt, C.; Krickemeyer, E.; Schmidtmann, M.; B€ogge, H.; K€ogerler, P.; Kim, T.; Luong, K.; M€uller, A. Angew. Chem., Int. Ed. 2002, 41, 2805–2808. (i) Howell, R. C.; Perez, F. G.; Jain, S.; Horrocks, W. D., Jr.; Rheingold, A. L.; Francesconi, L. C. Angew. Chem., Int. Ed. 2001, 40, 4031–4034. (j) M€uller, A.; Beugholt, C.; B€ogge, H.; Schmidtmann, M. Inorg. Chem. 2000, 39, 3112–3113. (20) Peacock, R. D.; Weakley, T. J. R. J. Chem. Soc. A 1971, 1836–1839. (21) Sadakane, M.; Dickman, M. H.; Pope, M. T. Angew. Chem., Int. Ed. 2000, 39, 2914–2916. (22) Mialane, P.; Lisnard, L.; Mallard, A.; Marrot, J.; Antic-Fidancev, E.; Aschehoug, P.; Vivien, D.; Secheresse, F. Inorg. Chem. 2003, 42, 2102–2108. 4954
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
Inorganic Chemistry (23) Bassil, B. S.; Dickman, M. H.; von der Kammer, B.; Kortz, U. Inorg. Chem. 2007, 46, 2452–2458. (24) (a) Niu, J. Y.; Zhao, J. W.; Wang, J. P. Inorg. Chem. Commun. 2004, 7, 876–879. (b) Wang, J. P.; Zhao, J. W.; Niu, J. Y. Sci. China, Ser. B: Chem. 2005, 48, 343–351. (c) Wang, J. P.; Duan, X. Y.; Du, X. D.; Niu, J. Y. Cryst. Growth Des. 2006, 6, 2266–2270. (d) Wang, J. P.; Zhao, J. W.; Duan, X. Y.; Niu, J. Y. Cryst. Growth. Des. 2006, 6, 507–513. (25) An, H. Y.; Han, Z. B.; Xu, T. Q. Inorg. Chem. 2010, 49, 11403–11414. (26) Laronze, N.; Marrot, J.; Herve, G. Chem. Commun. 2003, 2360–2361. (27) Laronze, N.; Marrot, J.; Herve, G. Inorg. Chem. 2005, 44, 1275–1281. (28) Laronze, N.; Haouas, M.; Marrot, J.; Taulelle, F.; Herve, G. Angew. Chem., Int. Ed. 2006, 45, 145–148. (29) Laronze, N.; Marrot, J.; Herve, G. C. R. Chim. 2006, 9, 1467–1471. (30) (a) Bi, L.; Kortz, U. Inorg. Chem. 2004, 43, 7961–7962. (b) Nellutla, S.; Tol, J.; Dalal, N. S.; Bi, L.; Kortz, U.; Keita, B.; Nadjo, L.; Khitrov, G. A.; Marshall, A. G. Inorg. Chem. 2005, 44, 9795–9806. (31) Bassil, B. S.; Dickman, M. H.; Reicke, M.; Kortz, U.; Keita, B.; Nadjo, L. Dalton Trans. 2006, 4253–4259. (32) Teze, A.; Herve, G.; Finke, R. G.; Lyon, D. K. Inorg. Synth. 1990, 27, 85–135. (33) CrysAlis Pro; Oxford Diffraction Ltd.: Abingdon, U.K., 2007. (34) Sheldrick, G. M. Acta Crystallogr. 2008, A64, 112–122. (35) Liu, J. F.; Ortega, F.; Sethuraman, P.; Katsoulis, D. E.; Costello, C. E.; Pope, M. T. J. Chem. Soc., Dalton Trans. 1992, 1901–1906. (36) Chatterjee, R.; Ali, M.; Drew, M. G. B.; Nethaji, M.; Mondal, S.; Mukherjee, M. Transition Met. Chem. 2009, 34, 1–5. (37) Laronze, N.; Marrot, J.; Herve, G. Inorg. Chem. 2003, 42, 5857–5862. (38) Helm, L.; Merbach, A. E. Coord. Chem. Rev. 1999, 187, 151–181. (39) Favas, M. C.; Kepert, D. L. Prog. Inorg. Chem. 1981, 28, 309–367. (40) (a) Porai-Koshits, M. A.; Aslanov, L. A. Zh. Strukt. Khim. 1972, 13, 266–276. (b) Hoard, J. L.; Silverton, J. V. Inorg. Chem. 1963, 2, 235–243. (c) Kepert, D. L. J. Chem. Soc. 1965, 4736–4744. (d) Lippard, S. J.; Russ, B. J. Inorg. Chem. 1968, 7, 1686–1688. (e) Muetterties, E. L. Inorg. Chem. 1973, 12, 1963–1966. (41) (a) Corbett, J. D. Struct. Bonding (Berlin) 1997, 87, 157–193. (b) F€assler, T. F.; Hoffmann, R. Angew. Chem., Int. Ed. 1999, 38, 543–546. (42) Karraker, D. G. J. Chem. Educ. 1970, 47, 424–430. (43) (a) Brown, I. D.; Altermatt, D. Acta Crystalllogr., Sect. B 1985, 41, 244–247. (b) Trzesowska, A.; Kruszynski, R.; Bartczak, T. J. Acta Crystallogr., Sect. B 2004, 60, 174–178. (44) (a) Mialance, P.; Dolbecq, A.; Lisnard, L.; Mallard, A.; Marrot, J.; Secheresse, F. Angew. Chem., Int. Ed. 2002, 41, 2398–2401. (b) An, H. Y.; Wang, E. B.; Xiao, D. R.; Li, Y. G.; Su, Z. M.; Xu, L. Angew. Chem., Int. Ed. 2006, 45, 904–908. (c) Du, D. Y.; Qin, J. S.; Li, S. L.; Lan, Y. Q.; Wang, X. L.; Su, Z. M. Aust. J. Chem. 2010, 63, 1398–1395. (45) (a) Niu, J. Y.; Wang, K. H.; Chen, H. N.; Zhao, J. W.; Ma, P. T.; Wang, J. P.; Li, M. X.; Bai, Y.; Dang, D. B. Cryst. Growth Des. 2009, 9, 4362–4372. (b) Niu, J. Y.; Zhao, J. W.; Wang, J. P. Inorg. Chem. Commun. 2004, 7, 876–879. (46) (a) Binnemans., K.; G€orller-Walrand, C. Chem. Phys. Lett. 1995, 235, 163–174.(b) Carnall, W. T.; Goodman, G. L.; Rajnak, K.; Rana, R. S. Argonne National Laboratory Report NL-88-8; Argonne National Laboratory: Argonne, IL, 1988. (47) (a) Yamase, T. Chem. Rev. 1998, 98, 307–325. (b) Papaconstantinou, E. Chem. Soc. Rev. 1989, 18, 1–31. (48) (a) Xia, J.; Zhao, B.; Wang, H.-S.; Shi, W.; Ma, Y.; Song, H. B.; Cheng, P.; Liao, D. Z.; Yan, S. P. Inorg. Chem. 2007, 46, 3450–3458. (b) Lill, D. T.; Bettencourt-Dias, A.; Cahill, C. L. Inorg. Chem. 2007, 46, 3960–3965. (49) (a) Xu, Q. H.; Li, L. S.; Liu, X. S.; Xu, R. R. Chem. Mater. 2002, 14, 549–555. (b) Yan, B.; Bai, Y. Y. J. Fluoresc. 2005, 15, 605–611.
ARTICLE
(50) (a) Kuang, J. Y.; Liu, Y. L.; Zhang, J. X. J. Solid State Chem. 2006, 179, 266–269. (b) Meshova, S. B.; Kiriyaka, A. V.; Tsvirko, M. P.; Gorodnyuk, V. P. J. Anal. Chem. 2008, 63, 840–843. (51) Sadakane, M.; Steckhan, E. Chem. Rev. 1998, 98, 219–237. (52) (a) Xi, X. D.; Wang, G.; Liu, B. F.; Dong, S. J. Electrochim. Acta 1995, 40, 1025–1029. (b) Liu, L. Z.; Li, F. Y.; Xu, L.; Liu, X. Z; Gao, G. G. J. Solid State Chem. 2010, 183, 350–355.
4955
dx.doi.org/10.1021/ic2001943 |Inorg. Chem. 2011, 50, 4944–4955
